1) Using the data in the table, which of the conjugate acids below is the strongest acid?
A) NH4
+
B) C5H5NH+
C) H3NOH+
D) NH3CH3
+
E) NH4
+ and NH3CH3
+
2) A substance with unpaired electrons will be ________.
A) slightly attracted to a magnet
B) slightly repelled by a magnet
C) permanently magnetic
D) brightly colored
E) nonmetallic
3) The hybrid orbital set used by the central atom in PCl5 is ________.
A) sp
B) sp2
C) sp3
D) sp3d
E) sp3d2
4) A freshly prepared sample of curium-243 undergoes 3312 disintegrations per second.
After 8.00 yr, the activity of the sample declines to 2591 disintegrations per second. The
half-life of curium-243 is
A) 6.26
B) 32.6
C) 10.2
D) 1.36
E) 22.6
5) The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base?
A) 2.1 x 10-4
B) 4.4 x 10-8
C) 8.8 x 10-8
D) 6.6 x 10-4
E) 2.0 x 10-5
6) ________ typically form ions with a 2+ charge.
A) Alkaline earth metals
B) Halogens
C) Chalcogens
D) Alkali metals
E) Transition metals
7) Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide:
PbCO3 (s) → PbO (s) + CO2 (g)
If the reaction yield is 95.7%, how many grams of lead (II) oxide will be produced by
the decomposition of 2.50 g of lead (II) carbonate?
A) 1.04
B) 1.55
C) 2.18
D) 4.00
E) 5.55
8) The oxidation number of xenon in XeF4 is ________.
A) +4
B) +3
C) +5
D) +1
E) -6
9) A mixture of He and Ne at a total pressure of 0.95 atm is found to contain 0.32 mol
of He and 0.56 mol of Ne. The partial pressure of Ne is ________ atm.
A) 1.7
B) 1.5
C) 0.60
D) 0.35
E) 1.0
10) The element calcium is in a group known as the _______.
A) transition metals
B) alkali metals
C) halogens
D) noble gases
E) alkaline earth metals
11) Why don’t we draw double bonds between the Be atom and the Cl atoms in BeCl2?
A) That would give positive formal charges to the chlorine atoms and a negative formal
charge to the beryllium atom.
B) There aren’t enough electrons.
C) That would result in more than eight electrons around beryllium.
D) That would result in more than eight electrons around each chlorine atom.
E) That would result in the formal charges not adding up to zero.
12) There are ________ ng in a pg.
A) 0.001
B) 1000
C) 0.01
D) 100
E) 10
13) The solubility of lead (II) chloride (PbCl2) is 1.6 x 10-2 M. What is the Ksp of
PbCl2?
A) 5.0 x 10-4
B) 4.1 x 10-6
C) 3.1 x 10-7
D) 1.6 x 10-5
E) 1.6 x 10-2
14) What form of hemoglobin is purplish-red?
A) myoglobin
B) deoxyhemoglobin
C) heme
D) oxyhemoglobin
E) none of the above
15) If the reaction yield is 94.4%, what mass in grams of hydrogen is produced by the
reaction of 4.73 g of magnesium with 1.83 g of water?
Mg (s) + 2H2O (l) → Mg(OH)2 (s) + H2 (g)
A) 0.0962
B) 0.0162
C) 0.0485
D) 0.219
E) 0.204
16) The correct name for CaO is ________.
A) calcium oxide
B) calcium hydroxide
C) calcium peroxide
D) calcium monoxide
E) calcium dioxide
17) The correct ground-state electron configuration for molybdenum is ________.
A) [Kr]5s14d10
B) [Kr]5s24d4
C) [Kr] 5s14d5
D) [Kr]5s24d5
E) [Kr]5s24d9
18) Which element forms an ion with the same charge as the sulfate ion?
A) magnesium
B) sodium
C) fluorine
D) vanadium
E) sulfur